What is the molarity of a solution that contains 133.6 g NaCl (molar mass = 58.44 g/mol) in 3.2 L solution

To find the molarity (M) of a solution, we use the formula:

\[
M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}
\]

### Step 1: Calculate the moles of NaCl
We are given the mass of NaCl as 133.6 g and its molar mass as 58.44 g/mol. To find the moles of NaCl:

\[
\text{moles of NaCl} = \frac{\text{mass of NaCl}}{\text{molar mass of NaCl}} = \frac{133.6 \, \text{g}}{58.44 \, \text{g/mol}} = 2.286 \, \text{mol}
\]

### Step 2: Calculate the molarity
The volume of the solution is 3.2 L, and we now know the moles of NaCl. So, the molarity (M) is:

\[
M = \frac{2.286 \, \text{mol}}{3.2 \, \text{L}} = 0.714 \, \text{M}
\]

Thus, the molarity of the solution is **0.714 M**.

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Would you like more details on any part of the calculation?

Here are five related questions to think about:
1. How would the molarity change if the volume of the solution were doubled?
2. What would the molarity be if you used 50 g of NaCl in the same volume of solution?
3. How can you dilute a 0.714 M solution to make a 0.5 M solution?
4. How does temperature affect the molarity of a solution?
5. What would happen if 133.6 g of KCl (molar mass = 74.55 g/mol) were dissolved in 3.2 L?

**Tip**: Always ensure your volume is in liters when calculating molarity!

What is the molarity of a solution that contains 133.6 g NaCl (molar mass = 58.44 g/mol) in 3.2 L solution?

Learn how to calculate the molarity of a NaCl solution containing 133.6 g of NaCl (molar mass 58.44 g/mol) dissolved in 3.2 L of solution. The step-by-step solution shows key concepts like molarity, moles, and unit conversions. Suitable for high school chemistry students in Grades 10-12.

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